S.MORRIS 2006. Papercuts This piece of paper is 28cm x 2.5 cm How many times would you have to cut...
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Transcript of S.MORRIS 2006. Papercuts This piece of paper is 28cm x 2.5 cm How many times would you have to cut...
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S.MORRIS 2006
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Papercuts
• This piece of paper is 28cm x 2.5 cm• How many times would you have to cut this
piece of paper to be the same width as an atom?• Once you cut a piece in half, you have to discard
one half and then use the other piece to continue this process
• Repeat this until you can no longer cut the paper.
• How many cuts did you make?
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Width of an Atom
• The average width of an atom is 130 picometers
• 1pm = 10-12 m = 1/1 000 000 000 000 of a meter
• 1 millimeter = 1 000 000 000 picometers
• That’s teeny tiny !
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Who are these dead dudes?
How did they contribute to our
present day model of an atom?
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HISTORY OF THE ATOMHISTORY OF THE ATOM
460 BC Democritus develops the idea of atoms
he pounded up materials in his pestle and
mortar until he had reduced them to
smaller and smaller particles which he
called
ATOMAATOMA
(greek for indivisible)
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This theory was ignored and forgotten for more than 2000 years!
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HISTORY OF THE ATOMHISTORY OF THE ATOM
1808 John Dalton
suggested that all matter was made up of
tiny spheres that were able to bounce
around with perfect elasticity and called
them
ATOMSATOMS
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Dalton’s Theory 1. all elements are composed of atoms.
2. atoms of the same element are exactly alike.
3. atoms of different elements are different.
4. compounds are formed by the joining of atoms of two or more elements.
Fill this in on your Notes sheet
Dalton’s Atom
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HISTORY OF THE ATOMHISTORY OF THE ATOM
1898 Joseph John Thompson
found that atoms could sometimes eject a
far smaller negative particle which he
called an
ELECTRONELECTRON
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HISTORY OF THE ATOMHISTORY OF THE ATOM
Thompson develops the idea that an atom was made up of
electrons scattered unevenly within an elastic sphere
surrounded by a soup of positive charge to balance the
electron's charge
1904
like plums surrounded by pudding.
PLUM PUDDING
MODEL
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HISTORY OF THE ATOMHISTORY OF THE ATOM
1910 Ernest Rutherford
oversaw Geiger and Marsden carrying out
his famous experiment.
they fired Helium nuclei at a piece of gold
foil which was only a few atoms thick.
they found that although most of them
passed through. About 1 in 10,000 hit
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HISTORY OF THE ATOMHISTORY OF THE ATOM
gold foil
helium nuclei
They found that while most of the helium nuclei passed
through the foil, a small number were deflected and, to
their surprise, some helium nuclei bounced straight back.
helium nuclei
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HISTORY OF THE ATOMHISTORY OF THE ATOM
Rutherford’s new evidence allowed him to propose a
more detailed model with a central nucleus.
He suggested that the positive charge was all in a
central nucleus. With this holding the electrons in place
by electrical attraction
However, this was not the end of the story.
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HISTORY OF THE ATOMHISTORY OF THE ATOM
1913 Niels Bohr
studied under Rutherford at the Victoria
University in Manchester.
Bohr refined Rutherford's idea by
adding that the electrons were in
orbits. Rather like planets orbiting the
sun. With each orbit only able to
contain a set number of electrons.
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The Bohr model was a modification of the Rutherford model.
Bohr the electrons in certain circular orbits around the nucleus called shells.
Bohr’s Atomic Theory
+
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Scientists had learned a lot about the atom, but couldn’t figure out what made it so
heavy. In 1932 James Chadwick solved the mystery by coming up with the idea of neutrons, neutral particles that
live in the nucleus with protons. The new improved Bohr model
includes these particles.
0
Neutrons
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Bohr Model of a HELIUM ATOM
+N
N
+-
-
proton
electron
neutron
Shell
New Bohr Model
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ATOMIC STRUCTUREATOMIC STRUCTURE
Particle
proton
neutron
electron
Charge
+ charge
- charge
No charge
1 amu
1 amunil
Mass
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Use your periodic table to help you Use your periodic table to help you find the ATOMIC STRUCTUREfind the ATOMIC STRUCTURE
the number of protons in an atom
the number of protons and neutrons in an atom
HeHe22
44 Atomic mass
Atomic number
Charge = # of protons + # of electrons
= (+ number) + (- number)
If the number of protons is the same as the number of electrons, what is the charge of the atom?
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ATOMIC STRUCTUREATOMIC STRUCTURE
Electrons are arranged in Energy Levels
or Shells around the nucleus of an atom.
• first shell a maximum of 2 electrons
• second shell a maximum of 8
electrons
• third shell a maximum of 8
electrons
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NucleusNucleus
11stst shell shell
22ndnd shell shell
33rdrd shell shell
Adapted from http://www.sciencespot.net/Media/atomsfam.pdf
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Created by G.Baker www.thesciencequeen.net
So let’s try it….• How to draw a Lithium atom
• First, look at the Periodic Table
• Second, How do you find the number of protons?
• Then determine the number of neutrons• Then determine the number of electrons
3
Li
Lithium
7
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Created by G.Baker www.thesciencequeen.net
So let’s try it….
3
Li
Lithium
7
++
++++
Protons = 3
Neutrons = 4
(7-3=4)
--
--
--
Electrons = 3 Electrons = 3
2 in the 12 in the 1stst shell, 1 in the shell, 1 in the 22ndnd shell shell